Reaction: 1 A + 1B = 3C The initial [A] is 1.20 M and [B] is 1.50 M. The equilibrium constant is 0.0000076. What is the concentration of C at equilibrium? You may assume the 5% rule is valid.

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O KINETICS AND EQUILIBRIUM Using the small x approximation to solve equilibrium problems A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 NO(g) + Cl,(g) 2 NOCI(g) K,=2. x 107 He fills a reaction vessel at this temperature with 8.0 atm of nitrogen monoxide gas and 9.7 atm of chlorine gas. Use this data to answer the guestions in the table below. O yes Can you predict the equilibrium pressure of NOCI, using only the tools available to you within ALEKS? O no If you said yes, then enter the equilibrium pressure of NOCI at right. Round your answer to 1 significant digit. atm II

Calculate the equilibrium concentrations for each reactant and product in the following equation at initial concentrations of 0.0400 M SO2, 0.0500 M NO2, 1.300 M NO and 0.200 M SO3.  The equilibrium constant for this reaction, Kc = 85.0. SO2(g) + NO2(g) ↔ NO(g) + SO3(g) Group of answer choices [SO2] = 0.0275, [NO2] = 0.0375, [NO] = 1.313, [SO3] = 0.213 [SO2] = 0.0309, [NO2] = 0.0409, [NO] = 1.309, [SO3] = 0.209 [SO2] = 0.0525, [NO2] = 0.0625, [NO] = 1.288, [SO3] = 0.188 [SO2] = 0.0491, [NO2] = 0.0591, [NO] = 1.291, [SO3] = 0.191

Consider the reaction A + B C+D, which has an equilibrium constant, K, equal to 3.4 x 102. If one begins a reaction by placing 0.600 moles of A in a 1.0 L container as well as 0.150 moles of 1. B, what will be the equilibrium concentrations of A, B, C, and D? Write your answers in the spaces provided below. a. [А] b. [B]= [C]= С. d. [D]= Once the reaction in problem 1 reaches equilibrium, some additional B is injected into the flask 2. from an outside source. LeChatelier's principle says the reaction will (circle one): be unchanged shift to the right shift to the left Pyridine is a weak base with a Kb 1.7 x 109. If 0.300 moles of pyridine is added to 1.00 L of 3. water, what will be the equilibrium concentrations of the species below: a. [Pyridine] = b. [Pyridine-H] (the pyridinium ion) [ОН-] 3 С. What is the pH of the solution in problem 4 (above)? .

Consider the reaction. PCI, (g) = PCI, (g) + Cl,(g) Ke = 0.0420 The concentrations of the products at equilibrium are [PC13] = 0.100 M and [Cl2] = 0.260 M. What is the concentration of the reactant, PCI5, at equilibrium? [PCI5] = M

Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2 HNO3(aq)+NO(9)→3 NO2(g)+H,0(1) At a certain temperature, a chemist finds that a 4.0 L reaction vessel containing a mixture of nitric acid, nitrogen monoxide, nitrogen dioxide, and water at equilibrium has the following composition: compound amount HNO3 5.2 g NO 19.8 g NO, 7.9 g H,O 134.3 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. °C K_ = 0 x10 C